XI Chemistry Chemical Equilibrium Online Test Mdcat-2024

Instructions for Chapter Chemical Equilibrium Online Test Mdcat-2024:

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Test Details:

Subject: Chemistry
Class: 1st year or 11
Chapter name: Chemical Equilibrium
Test: MDCAT 2024
Book: Sindh Textbook
Total No. Of MCQS: 50
Time Allowed: 50 Minutes
Price : Free

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Created on July 21, 2024 By

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XI Chemistry Chemical Equilibrium Online Test Mdcat-2024

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NameEmailPhone Number

1 / 50

1. Which of the following best describes a system in chemical equilibrium?

a) The concentration of reactants and products are equal.

b) The rate of the forward reaction is equal to the rate of the reverse reaction

c) The reaction has stopped completely.

d) The concentration of reactants is higher than the concentration of products.

2 / 50

2. Which of the following factors does NOT affect the position of equilibrium in a chemical reaction?

a) Temperature

b) Concentration of reactants

c) Presence of a catalyst

d) Pressure (for gases)

3 / 50

3. In the equilibrium expression Kc for the reaction ( aA + bB ⇌ cC + dD ), what does Kc represent?

a) The concentration of products divided by the concentration of reactants.

b) The sum of the concentrations of reactants and products.

c) The difference between the concentrations of reactants and products

d) The ratio of the concentration of reactants to products, each raised to the power of their coefficients.

4 / 50

4. Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust itself to:

a) Increase the disturbance.

b) Decrease the disturbance.

c) Completely stop the reaction.

d) Maintain the same concentrations of reactants and products

5 / 50

5. For the exothermic reaction, N₂(g) + 3H₂ (g) ⇌ 2NH₃ (g) what effect will increase the temperature have on the equilibrium position?

a) Shift to the right (towards products).

b) Shift to the left (towards reactants).

c) No effect.

d) Increase the rate of the forward reaction only.

6 / 50

6. Which of the following is a necessary condition for a chemical system to reach equilibrium?

a) The reaction must occur in an open system.

b) The temperature must remain constant.

c) The system must continuously add reactants.

d) The reaction must be endothermic.

7 / 50

7. Which condition is NOT required for a chemical system to achieve equilibrium?

a) Constant pressure (for gaseous reactions).

b) Constant concentration of reactants and products.

c) Equal rates of the forward and reverse reactions.

d) None

8 / 50

8. For the reaction ( aA + bB ⇌cC + dD ), if the concentrations of A and B are increased, what will be the effect on the equilibrium position according to the Law of Mass Action?

a) Shift to the left (towards reactants).

b) Shift to the right (towards products).

c) No change in the equilibrium position.

d) The reaction will stop.

9 / 50

9. Which of the following best describes the equilibrium constant ( Kc ) for a given reaction?

a) It is always a positive number.

b) It is always a negative number

c) It can be either positive or negative.

d) It is always zero

10 / 50

10. According to the Law of Mass Action, what happens to the equilibrium constant ( Kc ) when the temperature of an exothermic reaction is increased?

a) ( Kc ) increases.

b) ( Kc ) decreases.

c) ( Kc ) remains the same

d) ( Kc ) becomes zero.

11 / 50

11. In a reaction where the equilibrium constant ( Kc ) is very small, what does this indicate about the reaction?

a) The reaction favors the formation of products

b) The reaction favors the formation of reactants.

c) The reaction is very fast.

d) The reaction is very slow.

12 / 50

12. The Law of Mass Action can be used to:

a) Predict the speed of a reaction.

b) Determine the exact amounts of reactants and products at equilibrium.

c) Calculate the equilibrium concentrations of reactants and products if the equilibrium constant and initial concentrations are known.

d) Determine the molecular structure of the reactants and products.

13 / 50

13. For a given reaction at equilibrium, if the concentration of a product is increased, What will happen according to the Le Chatlier Principal?

a) The equilibrium will shift to the left (towards reactants).

b) The equilibrium will shift to the right (towards products).

c) The equilibrium constant ( Kc ) will increase.

d) The equilibrium constant ( Kc ) will decrease.

14 / 50

14. For the reaction ( 2A (g) + B(g) ⇌ 3C (g) ), the equilibrium concentrations are found to be [A] = 0.2M, [B] = 0.1M, and [C] = 0.6M. What is the value of the equilibrium constant ( Kc )?

a) 18

b) 54

c) 6

d) 0.18

15 / 50

15. For the reaction H₂(g) + I₂ (g) ⇌ 2HI (g) ), the initial concentrations are [H₂] = 1M, [I₂] = 1M, and [HI] = 0M. At equilibrium, the concentration of ( HI ) is 0.8 M. What is the value of ( Kc )?

a) 16

b) 4

c) 1

d) 8

16 / 50

16. Kp>Kc when :

a) Number of moles of reactant are more than no of moles of product

b) Number of moles of reactant are less than number of moles of product

c) Number of moles of product are less than number of moles of reactant

d) Number of moles of product are equal to number of moles of reactants

17 / 50

17. For the expression : H₂ + I₂ ⇌2HI, unit of Kc will be

a) dm⁶/mol²

b) dm³/mol

c) No unit

d) mol/ liter

18 / 50

18. If for a reaction Qc is 2 × 10־² and Kc is 1.3× 10־² then ?

a) Reaction will move in backward direction

b) Reaction will move in forward direction

c) Concentration of reactant will reduce till equilibrium is achieved

d) Both A and C

19 / 50

19. For a reaction involving gases, what does Delta n represent in the expression ( Kp = Kc (RT)^Δn )?

a) The difference in the number of moles of reactants.

b) The difference in the number of moles of products

c) The difference in the number of moles of gaseous products and reactants.

d) The sum of the moles of reactants and products.

20 / 50

20. If Kp is 5 for a reaction at 300 K and Δn= 1, what is the value of Kc? (Assume ( R = 0.0821 ) L·atm/(mol·K))

a) 5

b) 0.2

c) 20

d) 1

21 / 50

21. What is the relationship between Kp and Kx for a reaction involving gases at a constant total pressure?

a) Kx = Kp (RT)

b) Kx = Kp /(RT)

c) Kp=Kx(P)^Δn

d) Kp=Kx/P^Δn

22 / 50

22. Given the reaction ( H₂ (g) + I₂(g)⇌ 2HI (g) ) at equilibrium, if Kc = 50 at 400 K and Delta n = 0 , what is Kp ?

a) 50

b) 25

c) 100

d) 1

23 / 50

23. In a chemical reaction, what does it mean if ( Q = Kc )?

a) The reaction is moving in the forward direction.

b) The reaction is moving in the reverse direction.

c) The reaction is at equilibrium.

d) The reaction has not started.

24 / 50

24. Which of the following statements is true regarding the importance of Kc in predicting the extent of a reaction?

a) A very small Kc value indicates that the reaction strongly favors the formation of products.

b) A very large Kc value indicates that the reaction strongly favors the formation of reactants.

c) A Kc value close to 1 indicates that neither reactants nor products are favored.

d) Kc value is not important in predicting the extent of a reaction.

25 / 50

25. Why is the reaction quotient ( Qc ) useful in predicting the direction of a reaction?

a) It helps determine the energy released during the reaction.

b) It compares the current ratio of product and reactant concentrations to the equilibrium constant Kc .

c) It measures the speed of the reaction.

d) It indicates the pressure at which the reaction occurs.

26 / 50

26. According to Le Chatelier's principle, what happens to the equilibrium position if the concentration of a reactant is increased?

a) The equilibrium shifts to the left.

b) The equilibrium shifts to the right.

c) The equilibrium remains unchanged.

d) The reaction rate decreases.

27 / 50

27. For an exothermic reaction, how does an increase in temperature affect the equilibrium position?

a) Shifts to the right

b) Shifts to the left

c) Remains unchanged

d) Reaction rate increases

28 / 50

28. How does an increase in pressure affect the equilibrium of a gaseous reaction where the number of moles of gas decreases?

a) Shifts to the right

b) Shifts to the left

c) Remains unchanged

d) Reaction rate decreases

29 / 50

29. What happens to the equilibrium position when a catalyst is added to a reaction?

a) Shifts to the right

b) Shifts to the left

c) Remains unchanged

d) Reaction rate decreases

30 / 50

30. In the reaction N₂ (g) + 3H₂ (g) ⇌2NH₃ (g) ), how does decreasing the volume of the reaction vessel affect the equilibrium position?

a) Shifts to the right

b) Shifts to the left

c) Remains unchanged

d) Reaction rate decreases

31 / 50

31. For an endothermic reaction, how does a decrease in temperature affect the equilibrium position?

a) Shifts to the right

b) Shifts to the left

c) Remains unchanged

d) Reaction rate decreases

32 / 50

32. How does the removal of a product affect the equilibrium position of a reaction?

a) Shifts to the right

b) Shifts to the left

c) Remains unchanged

d) Reaction rate decreases

33 / 50

33. In a reversible reaction if certain amount of reactant is added then __ and reaction shift to___

a) Qc>Kc, right

b) Qc<Kc, left

c) Qc<Kc, right

d) Qc>Kc, left

34 / 50

34. Select the incorrect statement

a) A decrease of pressure shifts equilibrium in the direction of increased volume

b) Reversible reactions are exothermic in one direction and endothermic in other direction

c) Ammonia is synthesized by Haber’s process

d) None, as all are correct

35 / 50

35. Suitable condition for synthesis of Ammonia:

a) High Pressure

b) Low Temperature

c) Using catalyst (Fe)

d) All of these

36 / 50

36. The impurities of CaCl₂ and MgCl₂ of brine are removed by treating it with

a) CaCO₃

b) MgCO₃

c) Na₂CO₃

d) NaCO₃

37 / 50

37. What does the solubility product constant Ksp represent?

a) The concentration of a solute that dissolves in a solvent.

b) The product of the molar concentrations of the ions of a salt, each raised to the power of its coefficient in the balanced equation.

c) The rate at which a solute dissolves in a solvent.

d) The amount of solute that precipitates from a solution.

38 / 50

38. Which statement is true regarding the solubility of a salt when a common ion is added to the solution?

a) The solubility increases.

b) The solubility decreases.

c) The solubility remains the same.

d) The solubility product Ksp changes.

39 / 50

39. Select the incorrect statement

a) Ksp of a substance in saturated solution remains constant

b) Ksp changes with temperature

c) The product of molar concentration of the ions of two different salts is called solubility product

d) None,as all are correct

40 / 50

40. If solubility of BaSO₄ is given then it's Ksp can be found by:

a) Ksp = x²

b) Ksp = 4x³

c) Ksp =27x⁴

d) All of these

41 / 50

41. Which of the following best illustrates the common ion effect?

a) Adding NaCl to a saturated solution of AgCl and observing a decrease in the solubility of AgCl.

b) Adding NaNO₃ to a saturated solution of AgCl and observing an increase in the solubility of AgCl.

c) Adding more AgCl to its saturated solution and observing no change in solubility.

d) Adding water to a saturated solution of AgCl and observing an increase in solubility.

42 / 50

42. When Ksp>Qsp(Ionic Product) then the solution is said to be

a) Unsaturated

b) Saturated

c) Super Saturated

d) Unsaturated in which ppt is formed

43 / 50

43. What is a buffer solution?

a) A solution that speeds up chemical reactions.

b) A solution that resists changes in pH upon addition of small amounts of acid or base.

c) A solution that changes color when the pH changes.

d) A solution that completely neutralizes acids and bases.

44 / 50

44. Which of the following is a common example of an acidic buffer solution?

a) NH₃ and NH₄Cl

b) CH₃COOH and CH₃COONa

c) HCl and NaOH

d) NaOH and NaCl

45 / 50

45. What is the buffering capacity of a solution?

a) The ability to completely neutralize added acid or base.

b) The maximum amount of acid or base that can be added without a significant change in pH.

c) The change in pH upon addition of a small amount of acid or base.

d) The ratio of the concentrations of the conjugate base to the weak acid.

46 / 50

46. Acidic Buffer can be made by mixing of:

a) Strong Acid and it's salt with weak base

b) Strong Acid and it's salt with strong base

c) Weak Acid and it's salt with weak base

d) Weak Acid and it's salt with strong base

47 / 50

47. Basic Buffer can be made by mixing of :

a) Strong base and it's salt with weak acid

b) Weak base and it's salt with strong acid

c) Weak Acid And it's salt with strong base

d) Weak base and it's salt with weak acid

48 / 50

48. Which of the following is a common application of buffer solutions in biological systems?

a) Enhancing the rate of chemical reactions.

b) Maintaining a stable pH in blood.

c) Increasing the solubility of gases in water.

d) Preventing the evaporation of solvents.

49 / 50

49. Which buffer system is most commonly used to maintain the pH of blood?

a) Acetic acid and sodium acetate.

b) Ammonia and ammonium chloride.

c) Carbonic acid and bicarbonate.

d) Hydrochloric acid and sodium chloride.

50 / 50

50. Which of the following statements best describes the role of buffers in the food industry?

a) Buffers are used to enhance the taste of food products.

b) Buffers help maintain the pH of food products to prevent spoilage.

c) Buffers are added to food to increase its nutritional value.

d) Buffers help in the emulsification of fats.

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